Kinetics Flashcards
define rate of reaction
- how quickly a reaction happens
- the rate of change in concentration
- depends on how quickly the concentration of reactant or product changes with time
Rate of reaction equation
increase in product conc/ time taken
OR
decrease in reactant con/time taken
What unit is rate expressed in?
moldm-3s-1
What does a curved graph instead of a straight line tell us?
the gradient is not constant
How can you measure the rate of reaction on a graph?
draw a tangent to the curve at the time asked for
Why is the rate of reaction greater at the start of the reaction?
There is a greater reactant concentration
How would you measure rate of reaction if:
a. reaction produces colored precipitate
b. reaction produces gas
a. measure change in color
b. measure change in volume or mass of gas
Explain how to set up 2 experiments to measure the volume of gas produced.
- gas syringe moves outwards as gas collects
- gas collected by displacement of water from inverted burette. Gas has to have low solubility in water
Explain how to set up experiment measuring the change in mass.
- on digital balance, set beaker with cotton wool to prevent escape of liquid and solid
- but some gases are too light to show changes in mass
- needs continuous readings
kinetic molecular theory
particles in a substance move randomly because of the kinetic energy they possess
Do all particles in a substance have the same energy?
No. The random nature of movement and collisions means particles will have a range of energy values
What is the best way to measure the kinetic energy of a substance?
Take the average of the energy values of each molecule, and relate it to absolute temperature (temp measured in kelvin)
What does the Maxwell- Boltzmann distribution curve show?
Particles in a gas at a particular temperature show a range in their kinetic energy values
What is plotted on x and y axis in Maxwell-Boltzmann distribution curve?
x- kinetic energy
y- number of particles with kinetic energy
How do reactions occur?
- reactants placed together
- kinetic energy that particles possess cause them to collide with each other
- result: bonds between reactants broken, bonds form. Thus, products form
What is the collision theory?
- particles must collide
- particles must have sufficient energy
- particles must collide with correct orientation
What do many collisions lack?
Sufficient energy and correct orientation to break bonds of reactant
Activation Energy
energy required for reaction to take place
What are the factors affecting the rate of reaction?
- temperature
- concentration
- particle size
- pressure
- catalyst
Why is activation energy necessary?
- to overcome repulsion between molecules
- to break some bonds in reactants before they can react
Draw and label an endothermic graph
(look in book)
Draw and label an exothermic graph
(look in book)
Which particles can have successful collisions?
Particles that have a kinetic energy value greater than the activation energy will have successful collisions.
Do reactions with high or low activation energy proceed faster?
- high Ea reactions are slow
- low Ea reactions are faster